The concentration of `CO_(2)` in atmosphere is `88ppm`. If all of the `CO_(2)` present in `10^(5)mL` of air is dissolved in `1dm^(3)` water, then approximate `pOH` of solution at `27^(@)C` will be `(K_(a_(1)) = 10^(-7), K_(a_(2)) = 10^(-11)` for `H_(2)CO_(3)]`

In a solution of 0.1M H_(3)PO_(4) acid (Given K_(a_(1))=10^(-3),K_(a_(2))=10^(-7),K_(a_(3))=10^(-12)) Concentration of H_(2)PO_(4)^(-) is

What is the pH of 0.01 M glycine solution? For glycine, K_(a_(1))=4.5xx10^(-3) and K_(a_(2))=1.7xx10^(-10) at 298 K

Find the DeltapH( initial pH - final pH) when 100 ml 0.01M HCl is added in a solution containing 0.1m moles of NaHCO_(3) solution of negligible volume (k_(a_(1))=10^(-7),k_(a_(2))=10^(-11) for H_(2)CO_(3)) :

In a solution of 0.1M H_(3)PO_(4) acid Given K_(a_(1))=10^(-3),K_(a_(2))=10^(-7),K_(a_(3))=10^(-12)) Concentration of HPO_(4)^(2-) is

What is the pH of 0.01 M glycine solution? [For glycine, K_(a_(1))=4.5xx10^(-3) and K_(a_(2))=1.7xx10^(-10) at 298 K ]

In a solution of 0.1M H_(3)PO_(4) acid (Given K_(a_(1))=10^(-3),K_(a_(2))=10^(-7),K_(a_(3))=10^(-12)) pH of solution is

50 ml, 0.1M NaHCO_(3) aqueous solution is mixed with 50 ml, 0.8 M Na_(2)CO_(3) aqueous solution at 25^(@)C . The pH of resulting solution exiists between colour transition range of an indicator which is: (K_(a_(1))=4xx10^(-7), K_(a_(2)) =2xx10^(-11) "for" H_(2)CO_(3))

50 ml, 0.1M NaHCO_(3) aqueous solution is mixed with 50 ml, 0.8 M Na_(2)CO_(3) aqueous solution at 25^(@)C . The pH of resulting solution exiists between colour transition range of an indicator which is: (K_(a_(1))=4xx10^(-7), K_(a_(2)) =2xx10^(-11) "for" H_(2)CO_(3))

The pH of the a solution containing 0.4 M HCO_(3)^(-) is : [K_(a_(1)) (H_(2)CO_(3)) = 4 xx 10^(-7), K_(a_(2)) (HCO_(3)^(-)) = 4 xx 10^(-11)]